Calculate the molality of a 0.533 M aqueous solution of iron(II) chloride with a density, p = 1.059 g/mL. Report answer in three significant figures.
Calculate the molality of a 0.533 M aqueous solution of iron(II) chloride with a density, p = 1.059 g/mL. Report answer in three significant figures.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Calculate the molality of a 0.533 M aqueous solution of iron(II) chloride with a density, p = 1.059 g/mL. Report answer in three significant figures.
Expert Solution
Step 1
We have been given, a 0.533 M aqueous solution, means, the molarity is 0.533.
Molarity is the number of moles present per liter of the solution.
Also, density = 1.059 g/mL.
We have to find out molality of the solution which is number of moles of solute present per kg of the solution.
Given solute is iron(II) Chloride
Molar mass of solute = 127 g/mol
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